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Relevant bibliographies by topics / Hydrogen peroxide decomposition

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Academic literature on the topic 'Hydrogen peroxide decomposition'

Author: Grafiati

Published: 4 June 2021

Last updated: 18 February 2022

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Journal articles on the topic "Hydrogen peroxide decomposition"

1

TSUKADA, MASAO, AKIHIKO SEO, and TOMOAKI YOKOKURA. "The decomposition of hydrogen peroxide." Juntendo Medical Journal 50, no. 4 (2004): 515–22. http://dx.doi.org/10.14789/pjmj.50.515.

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Knotter, D. Martin, Stefan De Gendt, M. Baeyens, Paul W. Mertens, and Marc M. Heyns. "Hydrogen Peroxide Decomposition in Ammonia Solutions." Solid State Phenomena 65-66 (November 1998): 15–18. http://dx.doi.org/10.4028/www.scientific.net/ssp.65-66.15.

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Croiset, Eric, Steven F. Rice, and Russell G. Hanush. "Hydrogen peroxide decomposition in supercritical water." AIChE Journal 43, no. 9 (September 1997): 2343–52. http://dx.doi.org/10.1002/aic.690430919.

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Loeffler, M. J., and R. A. Baragiola. "Isothermal Decomposition of Hydrogen Peroxide Dihydrate." Journal of Physical Chemistry A 115, no. 21 (June 2, 2011): 5324–28. http://dx.doi.org/10.1021/jp200188b.

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Knotter, D. Martin, Stefan de Gendt, Martien Baeyens, Paul W. Mertens, and Marc M. Heyns. "Hydrogen Peroxide Decomposition in Ammonia Solutions." Journal of The Electrochemical Society 146, no. 9 (September 1, 1999): 3476–81. http://dx.doi.org/10.1149/1.1392499.

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Eberhardt, Manfred K., Angel A. Román-Franco, and Margarita R. Quiles. "Asbestos-induced decomposition of hydrogen peroxide." Environmental Research 37, no. 2 (August 1985): 287–92. http://dx.doi.org/10.1016/0013-9351(85)90108-2.

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Bourgeois, Marie-Josèphe, Marianne Vialemaringe, Monique Campagnole, and Evelyne Montaudon. "Réaction compétitive de la substitution homolytique intramoléculaire : décomposition de peroxydes allyliques dans le thioglycolate de méthyle." Canadian Journal of Chemistry 79, no. 3 (March 1, 2001): 257–62. http://dx.doi.org/10.1139/v01-024.

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The decomposition of allylic peroxides in methyl thioglycolate always leads to both epoxide and adduct peroxide. According to the nature of the allylic chain, either epoxide or peroxide is the predominant product, if not the only one. It is the first example where the hydrogen transfer is as fast as the intramolecular homolytic substitution. The influence of different factors upon the competition is studied.Key words: allylic peroxides, epoxides, intramolecular homolytic substitution, transfer.

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Watts, Richard J., Michael K. Foget, Sung-Ho Kong, and Amy L. Teel. "Hydrogen peroxide decomposition in model subsurface systems." Journal of Hazardous Materials 69, no. 2 (October 1999): 229–43. http://dx.doi.org/10.1016/s0304-3894(99)00114-4.

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Petigara, Bhakti R., Neil V. Blough, and Alice C. Mignerey. "Mechanisms of Hydrogen Peroxide Decomposition in Soils." Environmental Science & Technology 36, no. 4 (February 2002): 639–45. http://dx.doi.org/10.1021/es001726y.

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Hasegawa, Shinji, Kei Shimotani, Kentaro Kishi, and Hiroyuki Watanabe. "Electricity Generation from Decomposition of Hydrogen Peroxide." Electrochemical and Solid-State Letters 8, no. 2 (2005): A119. http://dx.doi.org/10.1149/1.1849112.

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Dissertations / Theses on the topic "Hydrogen peroxide decomposition"

1

Qiu, Zhiping. "Improvement in hydrogen peroxide bleaching by decreasing manganese-induced peroxide decomposition." Thesis, National Library of Canada = Bibliothèque nationale du Canada, 2000. http://www.collectionscanada.ca/obj/s4/f2/dsk1/tape3/PQDD_0034/MQ65515.pdf.

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Schmidt, Jeremy T. "Stabilized hydrogen peroxide decomposition dynamics in one-dimensional columns." Online access for everyone, 2006. http://www.dissertations.wsu.edu/Thesis/Spring2006/j%5Fschmidt%5F050306.pdf.

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Mitchell, Michael S. "Oxidation of biological molecules with bicarbonate-activated hydrogen peroxide and the decomposition of hydrogen peroxide catalyzed by manganese(II) and bicarbonate." [Gainesville, Fla.] : University of Florida, 2004. http://purl.fcla.edu/fcla/etd/UFE0004948.

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Widdis, Stephen. "Computational and Experimental Studies of Catalytic Decomposition of H2O2 Monopropellant in MEMS-based Micropropulsion Systems." ScholarWorks @ UVM, 2012. http://scholarworks.uvm.edu/graddis/239.

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The next generation of miniaturized satellites (“nanosats”) feature dramatically reduced thrust and impulse requirements for purposes of spacecraft attitude control and maneuvering. E↵orts at the University of Vermont have concentrated on developing a MEMS-based chemical micropropulsion system based on a rocket grade hydrogen peroxide (HTP) monopropellant fuel. A key component in the micropropulsion system is the catalytic reactor whose role is to chemically decompose the monopropellant, thereby releasing the fuel’s chemical energy for thrust production. The present study is a joint computational and experimental design e↵ort at developing a MEMS-based micro-reactor for incorporation into a monopropellant micropropulsion system. Numerically, 0D and simplified 2D models have been developed to validate the model and characterize heat and mass di↵usion in the channel. This model will then be extended to a 2D model including all geometric complexities of the catalyst bed geometry with the goal of optimization. Experimentally, both meso and micro scale catalyst geometries have been constructed to prove the feasibility of using RuO2 nanostructures as an in situ in a microchannel.

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Kwan, Wai P. (Wai Pang) 1974. "Kinetics of the Fe(III) initiated decomposition of hydrogen peroxide : experimental and model results." Thesis, Massachusetts Institute of Technology, 1999. http://hdl.handle.net/1721.1/80211.

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Kwan, Wai P. (Wai Pang) 1974. "Decomposition of hydrogen peroxide and organic compounds in the presence of iron and iron oxides." Thesis, Massachusetts Institute of Technology, 2003. http://hdl.handle.net/1721.1/29585.

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Thesis (Ph. D.)--Massachusetts Institute of Technology, Dept. of Civil and Environmental Engineering, 2003.
Includes bibliographical references.
Most advanced oxidation processes use the hydroxyl radical (OH) to treat pollutants found in wastewater and contaminated aquifers because OH reacts with numerous compounds at near diffusion-limited rates. OH can be made by reacting hydrogen peroxide (H202) with either Fe(II) (the Fenton reaction), Fe(1), or iron oxide. This dissertation investigated the factors that influence the decomposition rates of H202 and organic compounds, as well as the generation rate of -OH (VoH), in the presence of dissolved Fe(IH) and iron oxide. The Fe(III)-initiated chain reaction could be the dominant mechanism for the decomposition of H202 and organic compounds. The degradation rates of H14COOH, an OH probe, and H202 were measured in experiments at pH 4 containing either dissolved Fe(III) or ferrihydrite. Combined with the results from experiments using a radical chain terminator, we concluded that a solution chain reaction was important only in the Fe(III) system. In the ferrihydrite system the amount of dissolved Fe was insufficient to effectively propagate the chain reaction. In addition, a nonradical producing H202 loss pathway exists at the oxide surface. The oxidation rate of any dissolved organic compound can be predicted from VOH if the main sinks of -OH in the solution are known. Experiments using H14COOH and ferrihydrite, goethite, or hematite showed that VOH was proportional to the product of the concentrations of surface area and H202. Based on these results, a model was created for predicting the pseudo-first-order oxidation rate coefficients of dissolved organic compounds (korg) in systems containing iron oxide and H202. While our model successfully predicted korg in aquifer sand experiments, it yielded mixed results when compared to measurements from previously published studies.
(cont.) Some factors that could have caused the disagreements between model predictions and measurements were examined to refine our model. Results from experiments containing goethite, H 4COOH, and 2-Chlorophenol showed that H 4COOH detected more OH, which is produced at the oxide surface, than did 2-Chlorophenol. This was attributed to electrostatic attraction between the formate anions and the positively charged oxide surface, and could explain why our model, based on H14COOH, overpredicted the korg values of many neutral compounds.
by Wai P. Kwan.
Ph.D.

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Pakarinen, Darius. "On the mechanism of H2O2 decomposition on UO2-surfaces." Thesis, KTH, Skolan för kemi, bioteknologi och hälsa (CBH), 2018. http://urn.kb.se/resolve?urn=urn:nbn:se:kth:diva-240564.

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Deep geological repository has been investigated as a solution for long term storage of spent nuclear fuel in Sweden for more than 40 years now. The Swedish nuclear fuel and waste management company (SKB) are commissioning the deep repository and they must ensure that nuclear waste is isolated from the environment for thousands of years. During this time the containment must withstand physical stress and corrosion. It is important for a safety analysis to determine the different reactions that could occur during this time. If the physical barriers break down, radiolysis of water will occur. Hydrogen peroxide formed during the radiolysis can oxidize the exposed surface of the fuel, which increases the dissolution of radiotoxic products. Hydrogen peroxide can also catalytically decompose on the surfaces of the fuel. This project set out to figure out the selectivity for catalytic decomposition of hydrogen peroxide. This was to be done analytically with coumarin as a scavenger for detecting hydroxyl radicals formed when hydrogen peroxide decomposes. This produces the fluorescent 7-hydroxycoumarin that with high precision could be measured using spectrofluorometry. The results were giving approximately 0.16% ratio between •OH-production and hydrogen peroxide consumption. Similar experiments were done with ZrO2 for comparison, but the results were largely inconclusive. The effect of bicarbonate (a groundwater constituent) was also investigated. Adding bicarbonate increased the reproducibility of the experiments and increased the dissolution of uranium. Both the uranium and the bicarbonate increased the screening effects which minimized the fluorescent signal output by the 7-hydroxycoumarin.
Geologiskt djupförvar av förbrukat kärnbränsle har undersökts som lösning i Sverige i över 40 år nu. Svensk kärnbränslehantering (SKB) driftsätter det geologiska djupförvaret och måste säkerställa att det förbrukade kärnbränslet hålls isolerat från omgivningen i tusentals år. Under denna tid måste förseglingen stå emot fysikalisk stress och korrosion. Det är därför viktigt för en säkerhetsanalys att undersöka de olika reaktioner som kommer ske. Om förseglingen bryts ned kommer kärnbränslet i kontakt med vattnet i berggrunden vilket leder till radiolys av vatten. Väteperoxid som skapas under radiolysen kan sedan oxidera den exponerade ytan av kärnbränslet, detta ökar upplösningen av radiotoxiska produkter. Väteperoxiden kan även katalytisk sönderdelas på kärnbränslets yta. Syftet med arbetet var att få fram selektiviteten för katalytisk sönderdelning av väteperoxid. Detta skulle uppnås analytiskt med kumarin som avskiljare för detektion av hydroxylradikaler som bildas när väteperoxid sönderdelas. Detta producerade det fluorescerande 7-hydroxykumarinet som med hög precision kunde mätas spektrofluorometriskt. Resultaten gav en ca 0,16% förhållande mellan •OH-produktion och väteperoxidkonsumtion. Likartade experiment gjordes med ZrO2 för jämförelse men resultaten var ofullständiga. Effekten av bikarbonat (en beståndsdel i grundvatten) undersöktes också. Genom addition av bikarbonat ökade experimentens reproducerbarhet och ökade även upplösningen av uran. Både uranet och bikarbonaten minskade den utgående fluorescerande signalen från 7-hydroxykumarinet.

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Di, Menno Di Bucchianico Daniele. "The effect of solvent on the thermal and catalysed decomposition of hydrogen peroxide: an experimental and model analysis." Master's thesis, Alma Mater Studiorum - Università di Bologna, 2020.

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L'obiettivo di questo lavoro è quello di studiare l'effetto del solvente organico sulla decomposizione del perossido di idrogeno attraverso un'analisi sperimentale e di modellazione cinetica. L’analisi sperimentale esamina la decomposizione termica e la decomposizione catalizzata da γ-allumina in assenza e presenza di acetato di etile come solvente. Determinati attraverso cerimetria, i dati di concentrazione del perossido di idrogeno nei sistemi acquoso-solido e acquoso-organico-solido sono stati esaminati rispetto a parametri di reazione, come temperatura, massa di catalizzatore, rapporto in massa delle fasi acquosa-organica per i sistemi eterogenei-liquidi, e utilizzati nell’analisi di modellazione per definire modelli cinetici previsionali per la reazione di decomposizione nei diversi sistemi. Sulla base dei risultati sperimentali e cinetici, l'effetto del solvente sulla reazione di decomposizione del perossido di idrogeno è stato analizzato.

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Serra, Maia Rui Filipe. "Relation between surface structural and chemical properties of platinum nanoparticles and their catalytic activity in the decomposition of hydrogen peroxide." Diss., Virginia Tech, 2018. http://hdl.handle.net/10919/85149.

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The disproportionation of H₂O₂ to H₂O and molecular O₂ catalyzed by platinum nanocatalysts is technologically very important in several energy conversion technologies, such as steam propellant thrust applications and hydrogen fuel cells. However, the mechanism of H₂O₂ decomposition on platinum has been unresolved for more than 100 years and the kinetics of this reaction were poorly understood. Our goal was to quantify the effect of reaction conditions and catalyst properties on the decomposition of H₂O₂ by platinum nanocatalysts and determine the mechanism and rate-limiting step of the reaction. To this end, we have characterized two commercial platinum nanocatalysts, known as platinum black and platinum nanopowder, and studied the effect of different reaction conditions on their rates of H₂O₂ decomposition. These samples have different particle size and surface chemisorbed oxygen abundance, which were varied further by pretreating both samples at variable conditions. The rate of H₂O₂ decomposition was studied systematically as a function of H₂O₂ concentration, pH, temperature, particle size and surface chemisorbed oxygen abundance. The mechanism of H₂O₂ decomposition on platinum proceeds via two cyclic oxidation-reduction steps. Step 1 is the rate limiting step of the reaction. Step 1: Pt + H₂O₂ → H₂O + Pt(O). Step 2: Pt(O) + H₂O₂ → Pt + O₂ + H₂O. Overall: 2 H₂O₂ → O₂ + 2 H₂O. The decomposition of H₂O₂ on platinum follows 1st order kinetics in terms of H₂O₂ concentration. The effect of pH is small, yet statistically significant. The rate constant of step 2 is 13 times higher than that of step 1. Incorporation of chemisorbed oxygen at the nanocatalyst surface resulted in higher initial rate of H₂O₂ decomposition because more sites initiate their cyclic process in the faster step of the reaction. Particle size does not affect the kinetics of the reaction. This new molecular-scale understanding of the decomposition of H₂O₂ by platinum is expected to help advance many energy technologies that depend on the rate of H₂O₂ decomposition on nanocatalysts of platinum and other metals.
Ph. D.

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Rustin, Gavin James Mr. "The Analysis of the Decomposition of Hydrogen Peroxide Using a Schiff Base Copper Complex By Cyclic Voltammetry." Digital Commons @ East Tennessee State University, 2014. https://dc.etsu.edu/honors/224.

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Copper(II) complexes of Schiff bases can be used in the catalysis of hydrogen peroxide to create water and oxygen. The mechanism and the kinetics of this disproportionation reaction by a dimeric copper(II) complex [CuSALAD]2 are studied in this experiment, where SALAD refers to a Schiff Base ligand formed from salicyaldehyde and 1S,2S-D(+)-1-phenyl-2-amino-1,3-propanediol. By using cyclic voltammetry, the oxidation-reduction processes of a reaction may be monitored. The [CuSALAD]2 is initially reacted with a base such as imidazole to form the catalytic species, and the ratio of the copper(II) complex to the imidazole was found to be 1:4, consistent with previous electron absorption (UV-Vis) spectroscopy experiments. The reduction and oxidation half waves of the copper(II) catalyst are followed via cyclic voltammetry to determine if the copper(II) center undergoes reduction to copper(I) during the hydrogen peroxide catalysis. It appears that while the major oxidation and reduction half wave potentials, E1/2=6.51x10-2V, are unchanged during the decomposition, an additional oxidation wave (E1/2=1.43x10-1V) is observed in the absence of oxygen, suggesting some portion of the copper is reduced. With this information, a mechanism was proposed having copper as a catalyst and creating an intermediate that would form the water and the elemental oxygen.

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Books on the topic "Hydrogen peroxide decomposition"

1

Foget, Michael K. Goethite-catalyzed decomposition of hydrogen peroxide formulations: Implications for in situ bioremediation. 1992.

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Book chapters on the topic "Hydrogen peroxide decomposition"

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Ireneusz, Grubecki, and Zalewska Anna. "Optimal Feed Temperature for Hydrogen Peroxide Decomposition Process Occurring in the Reactor with Fixed-Bed of Commercial Catalase." In EngOpt 2018 Proceedings of the 6th International Conference on Engineering Optimization, 1434–45. Cham: Springer International Publishing, 2018. http://dx.doi.org/10.1007/978-3-319-97773-7_123.

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Bader, Klaus P., and Georg H. Schmid. "Photosynthetic Oxygen Evolution in the Filamentous Cyanobacterium Oscillatoria Chalybea: Interrelationship Between Water Splitting, Hydrogen Peroxide Decomposition and Nitrate Metabolism." In Nitrogen Fixation, 419–24. Dordrecht: Springer Netherlands, 1991. http://dx.doi.org/10.1007/978-94-011-3486-6_88.

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Lee, Gun Dae, Y. J. Do, Seong Soo Park, and Seong Soo Hong. "Effect of Hydrogen Peroxide on the Photocatalytic Decomposition of 4-Nitrophenol over TiO₂/Cr-Ti- MCM-41 Catalysts in Visible Light." In Materials Science Forum, 13–16. Stafa: Trans Tech Publications Ltd., 2005. http://dx.doi.org/10.4028/0-87849-966-0.13.

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Lowes, Bernard C. "Soil-Induced Decomposition of Hydrogen Peroxide." In In Situ Bioreclamation, 143–56. Elsevier, 1991. http://dx.doi.org/10.1016/b978-0-7506-9301-1.50013-5.

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Satapathy, P. K. "Decomposition of Aqueous Hydrogen Peroxide by Colloidal Manganese Dioxide." In Current Perspectives on Chemical Sciences Vol. 10, 162–68. Book Publisher International (a part of SCIENCEDOMAIN International), 2021. http://dx.doi.org/10.9734/bpi/cpcs/v10/5017d.

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Haines, R. I., D. R. McCracken, and J. B. Rasewych. "Poster 10. Decomposition of hydrogen peroxide under Candu coolant conditions." In Water chemistry of nuclear reactor systems 5, 1: 309–310. Thomas Telford Publishing, 1989. http://dx.doi.org/10.1680/wconrs5v1.15470.0050.

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"Tetrapyrrolic Macrocycles with Magnesium, Alluminum, and Zinc in Hydrogen Peroxide Decomposition." In Progress in Organic and Physical Chemistry, 139–48. Apple Academic Press, 2013. http://dx.doi.org/10.1201/b13964-17.

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Lin, C. C., F. R. Smith, N. Ichikawa, T. Baba, and M. Itow. "37. Decomposition of hydrogen peroxide in aqueous solutions at elevated temperatures." In Water chemistry of nuclear reactor systems 5, 1: 145–151. Thomas Telford Publishing, 1989. http://dx.doi.org/10.1680/wconrs5v1.15470.0022.

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Rebensdorff, B., and G. Wikmark. "38. Decomposition of hydrogen peroxide in high temperature water: a laboratory study." In Water chemistry of nuclear reactor systems 5, 1: 153–158. Thomas Telford Publishing, 1989. http://dx.doi.org/10.1680/wconrs5v1.15470.0023.

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Hiroishi, D., and K. Ishigure. "Poster 12. Homogeneous and heterogeneous decomposition of hydrogen peroxide in high-temperature water." In Water chemistry of nuclear reactor systems 5, 1: 311–312. Thomas Telford Publishing, 1989. http://dx.doi.org/10.1680/wconrs5v1.15470.0051.

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Conference papers on the topic "Hydrogen peroxide decomposition"

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Mok, Jong Soo, Jason Helms, and William Anderson. "Decomposition and Vaporization Studies of Hydrogen Peroxide." In 38th AIAA/ASME/SAE/ASEE Joint Propulsion Conference & Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2002. http://dx.doi.org/10.2514/6.2002-4028.

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Faraon, Victor A., Simona F. Pop, Raluca M. Senin, Sanda M. Doncea, and Rodica M. Ion. "Porphyrin-zeolite nanomaterials for hydrogen peroxide decomposition." In Advanced Topics in Optoelectronics, Microelectronics, and Nanotechnologies 2012, edited by Paul Schiopu and Razvan Tamas. SPIE, 2012. http://dx.doi.org/10.1117/12.966386.

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Corpening, Jeremy, Stephen Heister, Willam Anderson, and Benjamin Austin. "A Model for Thermal Decomposition of Hydrogen Peroxide." In 40th AIAA/ASME/SAE/ASEE Joint Propulsion Conference and Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2004. http://dx.doi.org/10.2514/6.2004-3373.

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Mok, J. S., J. Sisco, and W. Anderson. "Analysis and Experiments of Hydrogen Peroxide Vaporization and Decomposition." In 39th AIAA/ASME/SAE/ASEE Joint Propulsion Conference and Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2003. http://dx.doi.org/10.2514/6.2003-4621.

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Kwon, Hyuckmo, Seongmin Rang, and Sejin Kwon. "Study of Catalytic Decomposition for Hydrogen Peroxide Gas Generator." In 41st AIAA/ASME/SAE/ASEE Joint Propulsion Conference & Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2005. http://dx.doi.org/10.2514/6.2005-4458.

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Long, Matthew, and John Rusek. "The characterization of the propulsive decomposition of hydrogen peroxide." In 36th AIAA/ASME/SAE/ASEE Joint Propulsion Conference and Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2000. http://dx.doi.org/10.2514/6.2000-3683.

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Krejci, David, Alexander Woschnak, Carsten Scharlemann, and Karl Ponweiser. "Hydrogen Peroxide Decomposition for Micro Propulsion: Simulation and Experimental Verification." In 47th AIAA/ASME/SAE/ASEE Joint Propulsion Conference & Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2011. http://dx.doi.org/10.2514/6.2011-5855.

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Palmer, Matthew, Antony Musker, and Graham Roberts. "Experimental Assessment of Heterogeneous Catalysts for the Decomposition of Hydrogen Peroxide." In 47th AIAA/ASME/SAE/ASEE Joint Propulsion Conference & Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2011. http://dx.doi.org/10.2514/6.2011-5695.

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Farhat, Kamal, Yann Batonneau, Charles Kappenstein, and Marie Théron. "Decomposition of hydrogen peroxide: influence of the shape of catalyst support." In 46th AIAA/ASME/SAE/ASEE Joint Propulsion Conference & Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2010. http://dx.doi.org/10.2514/6.2010-6985.

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Bramanti, Cristina, Angelo Cervone, Luca Romeo, Lucio Torre, Luca d'Agostino, Antony J. Musker, and Giorgio Saccoccia. "Experimental Characterization of Advanced Materials for the Catalytic Decomposition of Hydrogen Peroxide." In 42nd AIAA/ASME/SAE/ASEE Joint Propulsion Conference & Exhibit. Reston, Virigina: American Institute of Aeronautics and Astronautics, 2006. http://dx.doi.org/10.2514/6.2006-5238.

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Reports on the topic "Hydrogen peroxide decomposition"

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Walsh, Raymond F., and Alan M. Sutton. Pressure Effects on Hydrogen Peroxide Decomposition Temperature. Fort Belvoir, VA: Defense Technical Information Center, August 2002. http://dx.doi.org/10.21236/ada405753.

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Sengupta, Debasis, Sandip Mazumder, J. V. Cole, and Samuel Lowry. Controlling Non-Catalytic Decomposition of High Concentration Hydrogen Peroxide. Fort Belvoir, VA: Defense Technical Information Center, February 2004. http://dx.doi.org/10.21236/ada426795.

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